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Chemistry
Q:
The following drawing is a representation of a reaction of the type A -> B, where different shaded spheres represent different molecular structures. For this reaction H = -30 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
The following drawing is a representation of a reaction of the type A -> B, where different shaded spheres represent different molecular structures. For this reaction H = +45 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
The following drawing is a representation of the exothermic reaction in which ozone forms dioxygen.What are the signs of H and S for this reaction?A) H = +, S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
The reaction represented in the above drawing is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and non spontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
What are the signs of H and S for the reaction represented in the above drawing?A) H = +, S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
The reaction represented in the above drawing is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and non spontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
are the signs of H and S for the reaction represented in the above drawing?A) H = +, S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -, G = -C) H = -, S = +,G = -D) H = -, S = -, G = -
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -, G = -C) H = -, S = +, G = -D) H = -, S = -, G = -
Q:
What are the signs of H, S, and G for the following spontaneous change?A) H = +, S = +, G = -B) H = +, S = -, G = -C) H = -, S = +, G = -D) H = -, S = -, G = -
Q:
The intermediate, T, + S is represented byA) arrow C.B) line D.C) line E.D) line F.
Q:
The product, Z, is represented byA) arrow A.B) line D.C) line E.D) line F.
Q:
The reactants, R + 2 S, are represented byA) arrow B.B) line D.C) line E.D) line F.
Q:
The net reaction is represented byA) arrow A.B) arrow B.C) arrow C.D) line F.
Q:
Step (2) in the reaction is represented byA) arrow A.B) arrow B.C) arrow C.D) 3line E.
Q:
Reactant R reacts with reactant S in two steps to yield product Z.Step (1) in the reaction is represented byA) arrow A.B) arrow B.C) arrow C.D) line E.
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done, and what is the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done, and what is the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
Imagine a reaction that results in a change in both volume and temperature, as shown in the diagram below. What is the sign of the work being done and the sign of the enthalpy change involved in this reaction?A) w = + and H = +B) w = + and H = -C) w = - and H = +D) w = - and H = -
Q:
The enthalpy of fusion of naphthalene, C10H8, is 19.1 kJ/mol at 78.2C, its melting point. Calculate the entropy of fusion at the melting point.A) Sfus = 244 J/(K mol)B) Sfus = 54.4 J/(K mol)C) Sfus = 1.49 J/(K mol)D) Sfus = -1.49 J/(K mol)
Q:
Calculate G for the reaction below and tell whether it is spontaneous or nonspontaneous under standard conditions at 25C.2 S (s) + 3 O2 (g) + 2 H2O (l) -> 2 H2SO4 (l) H = -1056 kJ/molS= -505 J/molA) G = -1207 kJ and the process is spontaneous.B) G = -1207 kJ and the process is nonspontaneous.C) G = -906 kJ and the process is spontaneous.D) G = -906 kJ and the process is nonspontaneous.
Q:
For the conversion of water to ice at 25C and 1 atm,A) G is negative and H is negative.B) G is negative and H is positive.C) G is positive and H is negative.D) G is positive and H is positive.
Q:
For the conversion of ice to water at 0C and 1 atm,A) G is zero, H is positive, and S is negative.B) G is zero, H is positive, and S is positive.C) G is negative, H is negative, and S is positive.D) G is positive, H is negative, and S is positive.
Q:
He gas is contained in a one-liter flask that is connected to an empty one-liter flask with a closed stopcock between the two flasks. When the stopcock is opened some of the He enters the evacuated flask. For this systemA) H is negative and S is positiveB) H is zero and S is positiveC) H is zero and S is negativeD) H is positive and S is negative
Q:
Methanol can be produced from carbon monoxide and hydrogen with suitable catalysts:CO(g) + 2 H2(g) -> CH3OH(l) at 25C H = -128.1 kJ and S = -332 J/K.Find G at 25C.A) -157.2 kJB) -29.1 kJC) 98.9 kJD) 157.2 kJ
Q:
When heated, mercury(II) oxide decomposes into elemental mercury and oxygen:2 HgO(s) -> 2 Hg(l) + O2(g) H = 181.6 kJ S = 216.4 J/KEstimate the temperature at which HgO should begin to decompose if the partial pressure of O2(g) is constant at 1.00 atm.A) -34.8CB) 34.8CC) 566CD) 840C
Q:
Consider the conversion of white tin to gray tin:Sn(white) -> Sn(gray) H = -2.09 kJ S = -7.41 J/Kbased on these data,A) white tin is stable below 9C and gray tin is stable above 9C.B) gray tin is stable below 9C and white tin is stable above 9C.C) white tin is stable below 15C and gray tin is stable above 15C.D) gray tin is stable below 15C and white tin is stable above 15C.
Q:
If a reaction with a negative value of S is nonspontaneous at constant temperature and pressure,A) G is negative and H may be positive or negative.B) G is negative and H is positive.C) G is positive and H may be positive or negative.D) G is positive and H is positive.
Q:
If an endothermic reaction is spontaneous at constant temperature and pressure,A) G is negative and S may be positive or negative.B) G is negative and S is positive.C) G is positive and S is negative.D) G is positive and S may be positive or negative.
Q:
What is the thermodynamic criterion for equilibrium for a reaction at constant temperature and pressure (PV work only)?A) S = 0B) G = 0C) S > 0D) G < 0
Q:
The reaction 4 Ag(s) + O2(g) -> 2 Ag2O(s) favors Ag2O at low temperature, but it favors Ag and O2 at high temperatures. How can this be explained in terms of H and S?A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
Which combination always results in a reaction being spontaneous?A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
Determine the sign of S for each of the following:I. The mixing of two gases at a given temperature and pressureII. C(s) + 2 H2O(g) -> CO2(g) + 2 H2(g)A) S is negative for I and negative for II.B) S is negative for I and positive for II.C) S is positive for I and negative for II.D) S is positive for I and positive for II.
Q:
Which of the following is not true?
A) A spontaneous reaction need not occur immediately.
B) A spontaneous reaction must be exothermic and must have an increase in entropy.
C) The reverse of a nonspontaneous reaction is always spontaneous.
D) A spontaneous reaction is one that can proceed on its own.
Q:
For the of freezing liquid ethanol at a given temperature and pressure,A) H is negative and S is negative.B) H is negative and S is positive.C) H is positive and S is negative.D) H is positive and S is positive.
Q:
Which thermodynamic function is most related to randomness?A) enthalpyB) internal energyC) entropyD) heat capacity
Q:
Determine the sign of S for each of the following:I. C6H6(s) -> C6H6(l)II. 2 SO2(g) + O2(g) -> 2 SO3(g)A) S should be negative for I and negative for II.B) S should be negative for I and positive for II.C) S should be positive for I and negative for II.D) S should be positive for I and positive for II.
Q:
In the redox reaction 2 S2O32-(aq) + I3-(aq) -> S4O62-(aq) + 3 I-(aq), if 18.75 mL of 0.2500 M Na2S2O3 is needed for complete reaction with 15.00 mL of the I3" solution, what is the molar concentration of I3"?
Q:
When the equation MnO4-(aq) + C2O42-(aq) -> Mn2+(aq) + CO2(g) is balanced using the smallest whole numbers, the coefficient in front of the CO2(g) is ________.
Q:
The reaction Cu(s) + 2 HCl(aq) -> CuCl2(aq) + H2(g) is predicted not to occur because Cu is ________ than H+ in the activity series.
Q:
In the reaction 2 MnO4-(aq) + 10 Br-(aq) + 16 H+(aq) -> 2 Mn2+(aq) +5 Br2(aq) + 8 H2O(aq) the reducing agent is ________.
Q:
The oxidation number of chromium in Na2Cr2O7 is ________.
Q:
In the reaction CH3CO2H(aq) + Ca(OH)2(aq) -> Ca(CH3CO2)2(aq) + 2 H2O(l)the acid is ________ and the base is ________.
Q:
Because it forms some H+ and OCl- ions when dissolved in water, the molecule HOCl is classified as a(n) ________.
Q:
The compound K2S is predicted to be soluble based on the solubility guideline that all ________ are soluble.
Q:
The balanced net ionic equation for the reaction Na2SO4(aq) + Pb(NO3)2(aq) -> PbSO4(s) + 2 NaNO3(aq) is ________.
Q:
CH3CO2H is an example of a ________ electrolyte.
Q:
What are the two products of the reaction H3PO4(aq) + 3 KOH(aq) -> ?
Q:
Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with theFe3+ present in the ore sample. The chemical equation for the reaction is2 Fe3+(aq) + Sn2+(aq) -> 2 Fe2+(aq) + Sn4+(aq).A) 5.365%B) 8.396%C) 16.79%D) 33.58%
Q:
Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.250 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) -> 6 Fe3+(aq) + Br-(aq) + 3 H2O(l).A) 0.0312 MB) 0.188 MC) 1.12 MD) 2.00 M
Q:
What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is2 S2O32-(aq) + I3-(aq) -> S4O62-(aq) + 3 I-(aq).A) 0.0833 MB) 0.120 MC) 0.167 MD) 0.333 M
Q:
Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the chemical equation:2 S2O32-(aq) + I3-(aq) -> S4O62-(aq) + 3 I-(aq).A) 6.22 mLB) 12.4 mLC) 24.9 mLD) 99.5 mL
Q:
According to the balanced equation shown below, 4.00 mole of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4-.5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) -> 10 CO2(g) + Mn2+(aq) + 8 H2O(l)A) 1.60B) 4.00C) 8.00D) 9.00
Q:
Using the following portion of the activity series for oxidation half reactions, determine which combination of reactants will result in a reaction.Na(s) -> Na+(aq) + e-Cr(s) -> Cr3+(aq) + 3 e-A) Na(s) with Cr(s)B) Na(s) with Cr3+(aq)C) Na+(aq) with Cr3+(aq)D) Na+(aq) with Cr(s)
Q:
How many electrons are needed for bromine in the balanced oxidation half-reaction?BrO3- (aq) + H+(aq) -> Br-(aq) + H2O(l)?A) -7B) -6C) +6D) +7
Q:
What is the oxidation number of the oxygen atom in Na2O2?
A) -2
B) -1
C) +1
D) +2
Q:
What is the oxidation number of the chromium atom in K2Cr2O4?
A) -2
B) +2
C) +6
D) +7
Q:
What is the oxidation number of the sulfur atom in K2SO4?
A) -2
B) +2
C) +4
D) +6
Q:
The chemical formula for nitrous acid is
A) H3N(aq).
B) HNO2(aq).
C) HNO3(aq).
D) H2N2O6(aq).
Q:
An aqueous solution of H2S is named
A) hydrosulfuric acid.
B) hydrosulfurous acid.
C) sulfuric acid.
D) sulfurous acid.
Q:
When dissolved in water, KOH behaves as
A) an acid that forms K+ and OH- ions.
B) an acid that forms KO- and H+ ions.
C) a base that forms K+ and OH- ions.
D) a base that forms KO- and H+ ions.
Q:
Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI, behave as bases when they are dissolved in water?
A) Ca(OH)2 and KOH
B) H2C2O4 and HI
C) only HI
D) only KOH
Q:
Which of the compounds of H2C2O4, Ca(OH)2, KOH, and HI, behave as acids when they are dissolved in water?
A) Ca(OH)2 and KOH
B) O4 and HI
C) only HI
D) only KOH
Q:
Which one of the following compounds behaves as an acid when dissolved in water?
A) RaO
B) C4H10
C) HI
D) RbOH
Q:
Which of the following compounds is an Arrhenius base?
A) CH3OH
B) CH3CO2H
C) HOCl
D) CsOH
Q:
Which of the following compounds is an Arrhenius base in water?
A) C6H12O6
B) HOCl
C) H2SO4
D) C6H5NH2
Q:
Which of the following compounds is not an Arrhenius acid?
A) CH3CO2H
B) CH3CH2NH2
C) HNO2
D) H2SO4
Q:
What reagent could not be used to separate Br- from CO32- when added to an aqueous solution containing both?
A) AgNO3 (aq)
B) Ca(NO3)2 (aq)
C) Cu(NO3)2 (aq)
D) Fe(NO3)2(aq)
Q:
What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both?
A) AgNO3 (aq)
B) Ba(OH)2 (aq)
C) CuSO4 (aq)
D) NaI (aq)
Q:
The mixing of which pair of reactants will result in a precipitation reaction?
A) Ba(NO3)2(aq) + Na2CO3(aq)
B) K2SO4(aq) + Cu(NO3)2(aq)
C) NaClO4(aq) + (NH4)2S(aq)
D) NH4Br(aq) + NH4I(aq)
Q:
The mixing of which pair of reactants will result in a precipitation reaction?
A) CsI(aq) + NaOH(aq)
B) HCl(aq) + Ca(OH)2(aq)
C) K2SO4(aq) + Hg2(NO3)2(aq)
D) NaNO3(aq) + NH4Cl(aq)
Q:
Which pair of compounds is soluble in water?
A) AgCl and AgBr
B) CoS and K2S
C) NaI and Cu(NO3)2
D) NH4NO3 and BaCO3
Q:
Which one of the following compounds is soluble in water?
A) Cu3(PO4)2
B) CoS
C) Pb(NO3)2
D) ZnCO3
Q:
Which one of the following compounds is insoluble in water?
A) CaCl2
B) NaNO3
C) PbCl2
D) K2CO3
Q:
What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution?
A) 0.150 M
B) 0.450 M
C) 1.35 M
D) 1.80 M
Q:
HCl, HI, H2SO4, LiCl, and KI are all classified as
A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
Q:
Based on the positions in the periodic table of elements A, B, and C, which of the following reactions would you expect to occur?A) A2+ + B -> A + B2+B) B2+ + C -> B + C2+C) C2+ + A -> C + A2+D) None of the reactions would be expected to occur.
Q:
Based on the positions in the periodic table of elements A, B, and C, which of the following reactions would you expect to occur?A) A2+ + B -> A + B2+B) B2+ + C -> B + C2+C) C + A -> C2- + A2+D) None of the reactions would be expected to occur.